(MBO) Oxidation Initiated by O(3P) - ACS Publications - American

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Low-Temperature Synchrotron Photoionization Study of 2‑Methyl-3buten-2-ol (MBO) Oxidation Initiated by O(3P) Atoms in the 298−650 K Range Yasmin Fathi, Chelsea Price, and Giovanni Meloni* Department of Chemistry, University of San Francisco, San Francisco, California 94117 United States S Supporting Information *

ABSTRACT: This work studies the oxidation of 2-methyl-3buten-2-ol initiated by O(3P) atoms. The oxidation was investigated at room temperature, 550, and 650 K. Using the synchrotron radiation from the Advanced Light Source (ALS) of the Lawrence Berkley National Laboratory, reaction intermediates and products were studied by multiplexed photoionization mass spectrometry. Mass-to-charge ratios, kinetic time traces, photoionization spectra, and adiabatic ionization energies for each primary reaction species were obtained and used to characterize their identity. Using electronic structure calculations, potential energy surface scans of the different species produced throughout the oxidation were examined and presented in this paper to further validate the primary chemistry occurring. Branching fractions of primary products at all three temperatures were also provided. At room temperature only three primary products formed: ethenol (26.6%), acetaldehyde (4.2%), and acetone (53.4%). At 550 and 650 K the same primary products were observed in addition to propene (5.1%, 11.2%), ethenol (18.1%, 2.8%), acetaldehyde (8.9%, 5.7%), cyclobutene (1.6%, 10.8%), 1-butene (2.0%, 10.9%), trans-2-butene (3.2%, 23.1%), acetone (50.4%, 16.8%), 3-penten-2-one (1.0%, 11.5%), and 3-methyl-2-butenal (0.9%, 2.5%), where the first branching fraction value in parentheses corresponds to the 550 K data. At the highest temperature, a small amount of propyne (1.0%) was also observed.

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INTRODUCTION Air pollution continues to be a leading threat to the environment. According to the Environmental Protection Agency (EPA), there are six common air pollutants: lead, ozone, particulate matter (PM), nitrogen oxides (NO2 and NO), sulfur dioxide (SO2), and carbon monoxide (CO).1 The burning of fossil fuels causes a dangerous amount of pollutants to be released in the atmosphere. The release of these gases are detrimental to the environment causing the earth’s climate to change.2 Fossil fuels have been used as the main source of energy throughout the past century. Petroleum-based gasoline emits constant air pollutants into the atmosphere that react with other compounds generating molecules harmful to human health and the environment. Fossil fuels are an expensive consumer product and have depleting resources.3 For this reason, researchers have been looking to find alternative sources for renewable energy and power transportation in a more affordable and earth friendly way.3 It has been found that the use of biofuels as an alternative fuel source produces less greenhouse gas emissions compared to fossil fuels4 (specifically, mixing ethanol with gasoline has been found to decrease carbon monoxide emissions5) and they are made from biomass that has been found as the only viable substitute.6 Popular renewable energy sources, biofuels, are slowly providing a long-term solution to reducing harmful combustion © XXXX American Chemical Society

emission of greenhouse gases. Most biofuels are oxygenated carbon-neutral hydrocarbons, made from a mix of different feedstock, such as vegetable oil, fats, and different greases.7 Oxygenated fuel increases the oxygen content in fuel while simultaneously reducing toxic emission.7 While biofuels express several benefits as a renewable energy source, however, in combustion, they can increase the emission of greenhouse gases such as nitrogen oxides and carbon oxides.8 Nonetheless, every biofuel reacts differently in the atmosphere and can create different byproducts that do not increase nitrogen oxide emissions. Short chain volatile alcohols are useful biofuels, which possess low water solubility and with linear hydrocarbon backbones, help confer combustion properties applicable in internal combustion engines.9 Nevertheless, the combustion of short chain volatile alcohols, used as biofuels, have become of great interest to observe what byproducts are formed in the atmosphere.9 In general, knowledge of their combustion is scarce. 2-Methyl-3-buten-2-ol (MBO) has become an attractive biofuel and renewable fuel additive due to its high energy content and low solubility in water.10 MBO is produced from Received: December 9, 2016 Revised: March 27, 2017 Published: March 31, 2017 A

DOI: 10.1021/acs.jpca.6b12421 J. Phys. Chem. A XXXX, XXX, XXX−XXX

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The Journal of Physical Chemistry A

Figure 1. Summation (blue line) of the literature photoionization spectra of ethenol (dark purple) and acetaldehyde (gray) superimposed onto the experimental photoionization curve at m/z 44 (pink line and open circles) at 298 K.

Figure 2. Comparison of the experimental photoionization curve of product m/z 58 superimposed onto the literature photoionization spectrum of acetone at 298 K.

the methyl erythritol-4-phosphate isoprenoid pathway.10 Up to this point, ethanol has been the popular short chain volatile alcohol used as a biofuel. MBO has a greater energy output, due to its higher energy density of 106 000 BTU gallon−1 (BTU = British thermal unit), much closer to petroleum gasoline 125 000 BTU gallon−1. Bioethanol on the other hand has a much lower energy content of 85 000 BTU gallon−1.10 Additionally, the low solubility in water helps purify the compound compared to ethanol allowing purified MBO to be captured of a culture without needed post harvesting.10 In this investigation, the O(3P) initiated oxidation reaction of MBO is studied to investigate potential byproducts that can be formed in combustion. Ground state oxygen atoms are spread throughout the atmosphere through combustion from engines.11 For this reason, researchers have found interest in how specific biofuels will react with O(3P). Cvetanovic began

researching the different pathways that occur initially in these type of reactions. He concluded that two main pathways might occur: an addition pathway to the less-substituted carbon atom of a multiple bond and a H atom abstraction where the O(3P) acts electrophilic.12,13 Two different studies have been done to further this finding, using multiplexed synchrotron photoionization mass spectrometry (MPIMS)14,15 and crossed molecular breams (CMBs),16 researchers concluded that at the beginning stages of the oxidation with O(3P) these reactions undergo intersystem crossing (ISC) taking the initial triplet reactant to singlet radical or intermediate leading to product formation. The MPIMS study of O(3P) with propene14,15 produced 40% of product formation from ISC, and the CBM study16 had almost 90% product formation from ISC. B


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Figure 3. Time trace of m/z 58 (red line and open triangles) superimposed onto the time trace of the reactant (dark brown and open circle) at 298 K. The time trace of the reactant has been multiplied by −1.

Figure 4. Literature photoionization spectra of NO (blue) superimposed onto the experimental photoionization curve at m/z 30 at 550 K (red line and open circles).

MBO (purity ≥98%) is commercially obtained from SigmaAldrich in liquid form, purified (freeze−pump−thaw technique), and along with helium gas is dispensed into a gas cylinder until the mixture has reached an overall partial pressure of 1%.19 Using calibrated mass flow controllers, the purified gas mixture enters into the heated slow flow quartz reactor tube.19 The mixture flows through a 650 μm pinhole directly into the ionization region, where it is photoionized via crossing tunable synchrotron radiation.19 The ground state oxygen atoms are generated through 351 nm photolysis of 1% NO2 and helium gas (NO2 → O(3P) + NO).17 According to Troe,20 at this wavelength the quantum yield of O(3P) is 1.00 and the absorption cross-section, according to Vandaele and coworkers21 is 4.62 × 10−19 cm2. On the basis of these values

The research presented here is carried out at room temperature, 550, and 650 K, using a tunable synchrotron multiplexed photoionization mass spectrometer, which has the ability to identify isomeric species via photoionization spectra. In addition, using electronic structure calculations potential energy surface scans of the different species produced throughout the oxidation are examined and presented.

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EXPERIMENTAL SECTION The synchrotron multiplexed time- and energy-resolved photoionization mass spectrometer at the Advanced Light Source (ALS) of Lawrence Berkeley National Lab has been previously described and, therefore, a brief explanation will be presented in this work.17−19 C


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Figure 5. Experimental photoionization spectrum of m/z 44 (dark yellow line and open circles) and the reference photoionization spectrum of propyne (purple line) for the MBO + O(3P) reaction at 650 K.

Figure 6. Literature photoionization spectra of propene (purple line) superimposed onto the experimental photoionization spectrum at m/z 42 (red line and dark yellow and open circles) at 550 and 650 K.

together with the concentration of NO2 of 1.3 × 1014 molecules cm−3 at 298 K, 3.7 × 1014 molecules cm−3 at 550 K, and 3.1 × 1014 molecules cm−3 at 650 K, and the laser fluence of 201 mJ cm−2, the concentration of O(3P) is held at 2.1 × 1013 molecules cm−3 at 298 K, 6.0 × 1013 molecules cm−3 at 550 K, and 5.1 × 1013 molecules cm−3 at 650 K. On the basis of the respective ionization energies, cations are formed and consequently accelerated and detected via a 50 kHz pulse orthogonal acceleration time-of-flight mass spectrometer.22,23 The mass resolution under the current experimental conditions is approximately 1,600.17 In this work the temperature of the reaction analyzed is varied and data is collected at 298, 550, and 650 K. Additionally, the pressures of these experiments are controlled using a feedback controlled throttle valve, starting at 4 Torr at 298 K and increasing to 7 Torr at both 550 and 650 K. These experiments results in a three-dimensional data plot that is integrated and sliced into two-dimensional data plots:

photon energy (eV) vs mass-to-charge ration (amu) and time (ms) vs mass-to-charge ratio (amu).24 Photoionization (PI) spectra are used to identify reaction intermediates and products formed throughout the oxidation. These spectra are obtained through the integration of the ion signal of a specific reaction time range yielding the plot of ion intensity as a function of photon energy. In this work, the photoionization spectra are integrated in the time range of 0−70 ms at 298 K, 0−30 ms at 550 K, and 0−10 ms at 650 K. The time intervals are chosen to minimize the presence of signal due to possible secondary reactions that might occur. Species identification is achieved by comparing the photoionization spectrum of detected products with either literature, calculated, or measured PI plots of species the products are believed to be. The AIE’s are determined by taking the linear extrapolation of the initial onset of the photoionization spectrum. The experimental adiabatic ionization energies have an estimated uncertainty of 0.05 eV for species identified with an onset. This uncertainty is due to the D


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Figure 7. (a) Summation (blue line) of the literature photoionization spectra of ethenol (purple line) and acetaldehyde (gray line) superimposed onto the experimental photoionization spectrum at m/z 44 (red line and open circles) at 550 K. (b) Reference photoionization spectrum of acetaldehyde and ethenol superimposed onto the experimental photoionization spectrum of m/z 44 at 650 K (dark yellow line and open circles).

and δ is the mass-discrimination factor, which has been determined to be equal to the mass of the identified species to the power of 0.67.25

photon energy step size, possible presence of hot bands, and energy resolution.19 The ion intensity over the whole photon energy range is integrated yielding a plot of ion intensity versus time. The time trace plots reveal the amount of reactant depleted or product formed over a certain time range of the oxidation. The primary products of this experiment are also identified via the comparison of their time traces with the depletion of the reactant. Secondary chemistry is observed when the product formation is slower than the reactant depletion. Once the reference photoionization spectra identify primary products at each observed signal, it is important to find the relative concentrations of each. Equation 1 shows the relation of the concentration (C) of a specific species at the photoionization spectrum intensity at a chosen energy (S(E)), in our experiments 11 eV. The instrumentation constant is k, σ represents the photoionization cross-section,

S(E) = kσ(E)δC

(1)

This work presents primary products observed from the oxidation of MBO + O(3P) with their corresponding branching fractions, which are the concentration of different products formed relative to the reactant. In order to perform this quantification, absolute photoionization cross sections, which are obtained through absolute photoionization spectra, are needed. The absolute photoionization spectrum of the reactant is acquired through comparing the known literature photoionization spectrum of propene at a known concentration with the experimental data. E


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Figure 8. Time trace of m/z 44 (red line and open triangles) superimposed onto the reactant time trace (dark brown and open circles) at 550 K. The time trace of the reactant has been multiplied by −1.

Sσ δ S σ (m )0.67 Sσ CP = P R R = P R R 0.67 = P R × MDF CR SR σPδ R S R σP SR σP(mP)

The branching fractions in eq 2 are derived measuring the ratio of the concentration of the product (CP) divided by the concentration of the reactant (CR) (measured as change in the initial reactant concentration) at a specified photon energy that is equal to the ratio of the product of the ion signal (product, SP, and reactant, SR), the photoionization cross-section (product, σP, and reactants, σR), and the mass discrimination factor (MDF).25 MDF is the quotient of reactant and product mass to the power of 0.67,25 which takes into account the massdependent response of the detector.

Once the products are identified, it is essential to determine the reaction pathways leading to the identified species from the initial oxidation. The potential energy surface scan is carried out as a function of bond lengths and bond angles using the B3LYP/6-31G(d) level of theory.33 The energies of stationary points (minima and transition states) are then recalculated using the CBS-QB3 method. These values are used to determine the enthalpy changes throughout the proposed mechanisms using MBO + O(3P) as the energy reference level. In order to further verify the forward and reverse steps of the different potential energy surface scans as well as the local minima and saddle points, intrinsic reaction coordinate (IRC) calculations are also performed.

COMPUTATIONAL INFORMATION The identification of products continues through electronic structure calculations. In this study, all computational calculations are completed in the Gaussian 0927 software suite using the CBS-QB3 composite model.28,26 This choice is based on its high accurate energetics with a mean absolute deviation of 1 kcal/mol and relative low computational cost.26 The AIE of the reaction species is obtained using the computed values of the corrected zero-point vibrational electronic energies of the ground state neutral and cationic species. These values are also used to calculate the enthalpy changes of proposed mechanism pathways leading to the products. The main focus of this research is to identify the products formed in combustion during the oxidation of MBO with O(3P). In most cases, reference photoionization spectra are available for comparison to the experimental data to verify which products are created. In the case, however, that a reference photoionization spectrum is unavailable, a photoelectron spectrum (PE) is simulated. The PE spectrum is generated using the Franck−Condon (FC) and Franck− Condon−Herzberg−Teller methods.29−31 The FC overlap integrals are calculated using recursive formula developed by Ruhoff.32 Once the photoelectron spectrum is computed, its integration will provide the simulated photoionization spectrum, which can be compared to the experimental photoionization curve at the specific signal for further product identification.

RESULTS To aid clarity to the discussion of the numerous observed reaction species and their pathways, the experimental data are first presented at the three temperature, 298, 550, and 650 K. A concise presentation of our quantitative results in form of branching fractions is then provided, followed by the computational characterization of the reaction pathways to substantiate the experimental findings. The oxidation with O(3P) yields two types of reactions: (1) oxygen addition and (2) hydrogen abstraction pathway. The most energetically favorable pathway is the O(3P) addition to either less-substituted carbon of the double bond. As seen in Scheme 1, triplet diradicals A and B are formed from the ground state oxygen atom adding to either unsaturated carbons. The enthalpy change (ΔrH) for radical A is −106 kJ/mol and for radical B is −109 kJ/mol. Diradical B (O(3P) addition to the secondary unsaturated carbon) is therefore a few kJ mol−1 more stable than A (O(3P) addition to the primary unsaturated carbon). These diradicals can enter the singlet surface through intersystem crossing (ISC) to form an epoxide that leads to several products observed in this study. The calculated ΔrH yielding the epoxide from the reactant is −370 kJ/mol. The epoxide cation is computed to be unbound using the CBS-QB3 model and, in fact, it has not been experimentally observed. The second type of reaction formed throughout this oxidation is the hydrogen abstraction from a methyl group bonded to the γ carbon (−5 kJ/mol). This radical is then attacked by O2

(2)

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F


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experimental ionization onset matches very well with the reference adiabatic ionization energy of 9.33 ± 0.01 eV for ethenol. The experimental ionization of acetaldehyde also is in good agreement with the literature adiabatic ionization energy of 10.20 ± 0.02 eV.35 The summation of the literature photoionization spectra of ethenol and acetaldehyde taken by Cool et al.36 matches very well with the experimental m/z 44 photoionization curve (Figure 1). Experimentally, the adiabatic ionization energy of acetone (m/z 58) is observed to be 9.70 ± 0.05 eV, compared to the literature adiabatic ionization energy of 9.694 ± 0.006 eV reported by Trott.37 In the absolute photoionization spectrum of MBO, m/z 58 is a dissociative photoionization fragment. However, in the studied reaction m/z 58 is observed as a product, i.e., its time trace is not depleting. The ratio of the dissociative photoionization fragment (daughter ion) and the reactant (parent ion) in the absolute photoionization spectrum (2.65 at 11 eV) is used to adjust the experimental m/z 58 spectrum. This is achieved by adding the normalized signal (with respect to the parent signal in the reaction data) of the daughter ion to the observed curve to take into account the depleting signal of the fragment. The resulting m/z 58 matches well to the literature photoionization spectrum of acetone within the very low signal-to-noise ratio, which affects the uncertainty of the measured ion signal as described in the section Branching Fractions (Figure 2).38 Acetone has been determined to be a primary product by comparing its kinetic trace to the temporal behavior of the reactant. Its time trace is presented in Figure 3. The time trace of the reactant, which is indeed a depleting signal, has been multiplied by −1 for comparison with the formation of the product. Product Identification of MBO + O(3P) at 550 and 650 K. At the higher temperatures, the oxidation of MBO presents additional products. At both temperatures, the following signals are identified: m/z 42, 44, 54, 56, 58, 70, 82, and 84. At 650 K, an additional primary product is identified at m/z 40. When photolyzing NO2 to create O(3P), NO is formed as well. At

Scheme 1. Three Radical Species Forming from the Initial MBO + O(3P) Reaction (the CBS-QB3 Calculated Enthalpy Changes Are Provided): The Two Oxy Radicals A and B, the H Abstraction Radical C, and the Peroxy Species D

forming a peroxide species (−254 kJ/mol). The last possible hydrogen abstraction for the ground state oxygen atom throughout this oxidation is from the alcohol group bonded to the γ carbon. However, it is an endothermic process with a calculated ΔrH of 5 kJ/mol and, thus, it is not considered in the analysis of the formation of the different species. MBO + O(3P) reactions are carried out at three different temperatures. At 298 K the measurements are performed from 9.3 to 11 eV, and at 550 and 650 K in the 8.7−11 eV range. Product Identification of MBO + O(3P) at 298 K. At room temperature, the oxidation of MBO + O(3P) forms only two signals at m/z 44, and m/z 58. The experimental photoionization spectrum at m/z 44 reveals two species. The experimental onset of the PI spectrum at 9.30 ± 0.05 eV agrees with the reference PI spectrum of ethenol up to around 10.20 eV, where the literature PI spectrum of acetaldehyde is matched. According to Ruscic and Berkowitz,34 the m/z 44

Figure 9. Experimental photoionization spectrum of m/z 54 at 550 (red line and open circles) and 650 K (dark yellow line and open circles) and the simulated Franck−Condon (FC) photoionization spectrum of cyclobutene (purple) for the MBO + O(3P) reaction. G


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Figure 10. Summation (blue line) of the literature photoionization spectra of trans-2-butene (purple) and 1-butene (gray) superimposed onto the experimental photoionization spectrum of m/z 56 at 650 K (dark yellow line and open circles) for the MBO + O(3P) reaction.

Figure 11. Experimental photoionization spectrum of m/z 70 at 550 (red line and open circles) and 650 K (dark yellow line and open circles) and the reference photoionization spectrum of 2-butenal (purple) for the MBO + O(3P) reaction.

multiplied by −1 for comparison with the formation of the product (Figure 8). The m/z 54 signal is assigned to cyclobutene (Figure 9) with its experimental AIE of 9.40 ± 0.05 eV in good agreement with the literature value of 9.43 ± 0.02 eV.42 There is no literature PI spectrum for cyclobutene, thus using the CBS-QB3 optimized geometries and force constants of the cationic and neutral species (Franck−Condon approximation), a photoelectron curve is simulated and integrated into a photoionization spectrum, which agrees with this study experimental data. Two isomeric species are formed at m/z 56 (Figure 10), trans2-butene and 1-butene. The ionization onset of 9.10 ± 0.05 eV is fit to the literature PI curve of trans-2-butene with a reported AIE of 9.10 ± 0.02 eV.43 The literature AIE of 1-butene of 9.62 ± 0.05 eV44 and Wang et al.45 PI spectrum agree well with the experimental data at the higher energy range. The summation of trans-2-butene and 1-butene spectra is a good match to the overall shape of the experimental signal at m/z 56 up to 10.1

signal m/z 30, the experimental photoionization spectrum matches very well to the reference photoionization spectrum of NO39 (Figure 4). A signal at m/z 40 is only observed at 650 K and assigned as propyne (Figure 5) based on the good agreement with its superimposed literature photoionization spectrum.38 The observed adiabatic photoionization energy is 10.40 ± 0.05 eV, which is in good agreement with the reported value of propyne of 10.37 ± 0.01 eV.40 Person and Nicole41 reference PI spectrum of propene agrees well with the experimental data at m/z 42 (Figure 6). The ionization onset of 9.70 ± 0.05 eV matches the reference AIE of 9.74 ± 0.0141 eV. Similarly to 298 K, products at m/z 44 are observed, however, the ethenol contribution gets smaller as the temperature is increased (Figure 7). Figure 8 presents the time trace of m/z 44 superimposed onto the time trace of the reactant at 550 K showing its fast formation as primary product. The time trace of the reactant (depleting signal) has been H


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Figure 13. Comparison of the experimental photoionization spectrum at m/z 82 superimposed onto the Franck−Condon simulation of the epoxide species at 550 K (red line and open circles) and 650 K (dark yellow line and open circles).

Figure 8 for comparison). The signal m/z 82 at both temperatures is assigned to cyclobutanecarbaldehyde based on the good match with the FC simulated spectrum (Figure 13). Finally, two nonisomeric species are characterized at m/z 84 (Figure 14). The ionization onset of the spectrum at 9.40 ± 0.05 eV is consistent with the measured spectrum of 3-penten2-one with a reported AIE of 9.39 eV.47 The spectrum of this species alone does not match the whole signal in the studied photoionization energy range. The inclusion of 3-methyl-2butenal with an AIE of 9.4 eV43 in the summation spectrum is in good agreement with the measured signal. Branching Fractions. The products formed at all three temperatures and their corresponding branching fractions, calculated using eq 2, are presented in Table 1. Both ion intensities and photoionization cross sections are a function of photon energy. For this reason, PI spectra of each product formed are compared at the same photon energy of 11 eV to

eV. At higher photon energies the unmatched experimental signal might be due to dissociative photoionization of products at m/z 84, which could undergo a CO loss. A product at m/z 58 is observed. The same procedure used at 298 K is applied at both 550 and 650 K to yield a signal consistent with the presence of acetone. m/z 70 is assigned to 2-butenal based on the good agreement of the observed ionization onset at 9.70 ± 0.05 eV with the literature AIE of 9.73 ± 0.01 eV46 and the literature spectrum (Figure 11).43 On the basis of the computational results presented below in the section Proposed Mechanism of MBO with O(3P), the formation of this species is not kinetically favorable due to a very high barrier for this formation. Therefore, this species cannot be considered to be a primary product. Figure 12 presents the time trace of m/z 70 superimposed onto the time trace of the reactant (multiplied by −1) at 550 K showing a slower formation than a primary product would have (see I


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Figure 14. Summation at 650 K (blue line) of the simulation Franck−Condon (FC) photoionization spectrum of 3-penten-2-one (purple line) and the literature photoionization spectrum of 3-methyl-2-butenal (gray line) superimposed onto the experimental photoionization spectrum at m/z 84 at 650 K (dark yellow line and open circles) for the MBO + O(3P) reaction.

Table 1. Branching Fractions of Products with Their Uncertainties Formed during the Oxidation of MBO Using O(3P) at 298, 550, and 650 K compound

m/z

298 K

550 K

650 K

From the O(3P) Addition Pathway propyne ethenol acetaldehyde trans-2-butene 1-butene acetone 3-penten-2-one 3-methyl-2-butenal

40 44 44 56 56 58 84 84

propene cyclobutene cyclobutanecarbaldehyde

42 54 82

26.6 ± 8.9 4.2 ± 1.5

53.4 ± 33.6

18.1 8.9 3.2 2.0 50.4 1.0 0.9

± ± ± ± ± ± ±

10.0 5.1 1.7 1.1 31.8 0.5 0.5

1.0 2.8 5.7 23.1 10.9 16.8 11.5 2.5

± ± ± ± ± ± ± ±

0.5 1.7 3.4 10.5 5.0 8.7 5.1 1.1

From the O(3P) H Abstraction Pathway 5.1 ± 2.8 1.6 ± 0.8 0.4 ± 0.3

11.2 ± 4.5 10.8 ± 4.7 2.4 ± 1.2

are also included. Technically, this pathway represents secondary chemistry in which only a fraction of the reactant, which is converted into the H-abstraction radical, reacts with some traces of O2 present in our experiment. Because we do not have a way to separate the two possible pathways (addition and abstraction), i.e., a way to quantify how much of MBO goes into each pathway, the values of the branching fractions can be a little different from the true values. If we knew the exact percentage of MBO reacting in each pathway, we could renormalize the branching fractions for this correct amount. Figure 15 presents the time trace of propene at 550 K superimposed onto the time trace of the reactant, showing a slower formation that is characteristic of secondary chemistry. Acetone with a branching fraction of 50.4 ± 31.8% is the major product at 550 K, whereas at 650 K trans-2-butene becomes the most abundant product with a branching fraction of 23.1 ± 10.5%. The relative amount of ethenol and acetone diminishes, as the temperature is increased. Proposed Mechanism of MBO with O(3P). As discussed above, the most favorable energetic pathway of the oxidation of MBO + O(3P) is the formation of the singlet epoxide from the

determine their concentrations. The uncertainties of the branching fractions are calculated using the propagation of errors of each variable in eq 2 and are listed in Table 1. The signal used to calculate the branching fractions at each temperature is average for 250 laser shots at each energy step. The uncertainties of the photoionization cross sections and the mass discrimination factor are from the literature, whereas the uncertainty of each ion signal is estimated by taking the difference between the measured upper value at 11 eV of a specific species and its reference (literature or simulation) spectrum used in the assignment. The same procedure is applied using the lower ion signal value at 11 eV. At 298 K, only three products are observed: ethenol, acetaldehyde, and acetone. They are quantified and the total branching fraction is 84.2 ± 34.8%. The large estimated error of the branching fraction of acetone (±33.6%) is due to the very low signal-to-noise ratio at m/z 58. At 550 and 650 K more products are observed and the overall branching fractions are 91.6 ± 33.9% and 98.7 ± 17.2%, respectively. In these overall values for the 550 and 650 K data the branching fractions of the products yielded from the H-abstraction radical + O2 pathway J


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barrier. E4 can undergo two different pathways. If hydrogen is transferred from the CH2 moiety to the adjacent C, a double bond is formed with a barrier of 14 kJ/mol (TS4a) yielding trans-2-butene and an enthalpy change of −278 kJ/mol. If instead hydrogen is transferred from the CH3 to the double radical C site, 1-butene is formed with a calculated barrier of 32 kJ/mol (TS4b) and enthalpy change of −279 kJ/mol (Figure 16a). In the second potential energy surface diagram (Figure 16b), further products are energetically proven through the singlet epoxide (F). Similarly, to the previous potential energy surface diagram, the initial oxidation of MBO with O(3P) is used as the reference point. The hydrogen transfer from the β carbon to the epoxidic oxygen yields a double radical site on the β carbon with a calculated enthalpy change of 238 kJ/mol (F1) and barrier of 285 kJ/mol (TS1). With a computed barrier of 58 kJ/ mol (TS2*), water is pulled off forming 3-methyl-2-butenal with an overall exothermicity of 298 kJ/mol. The hydrogen atom of the OH group from F1 can be transferred to the double radical to form F2 with a barrier of 30 kJ/mol (TS2) and enthalpy change of 243 kJ/mol. The βC-γC bond is cleaved yielding acetone and ethenol with a calculated enthalpy change of 25 kJ/mol and barrier of 239 kJ/mol (TS3*). Indeed, F2 has another fate; it can lead to the formation of 3-penten-2-one with an overall exothermicity of 276 kJ/mol. Since experimentally O2 is present in the 1% NO2 gas mixtures used to produce O(3P), O2 is considered for the mechanism of the formation of cyclobutene and propene. For this diagram shown in Figure 17, the radical plus the O2 is used as the reference point. Any transition state barrier above the red line is kinetically unfavorable throughout these pathways. The formation of the peroxy radical (D), O2 addition has a heat of reaction of −254 kJ/mol as seen previously. For the formation pathways of the three observed products, the initial step from D is the formation of D1 with an enthalpy change of −15 kJ/mol (D1). This species is not observed because it dissociatively ionizes according to our CBS-QB3 calculations. Cyclobutene is yielded through a high barrier (TS2*) 30 kJ/mol above the

triplet diradicals formed through the oxygen addition to the carbons of the double bond. The initial reaction of MBO with O(3P) forming triplet diradicals is used as the reference point for the energetic calculations of the products. Because of the numerous species computed in this oxidation, the products formed from the epoxide are separated into two different potential energy surface diagrams (a and b) (Figure 16). The epoxide is not seen throughout this reaction. Computationally its cation is unbound, conveying that the epoxide dissociatively ionizes. Any molecular species or energetic barrier above the red line in the potential energy surface diagrams is thermodynamically or kinetically unfavorable, respectively. In Figure 16a, the direction to right follows the formation of acetaldehyde and propyne and to the left it follows the formation of trans-2-butene and 1butene. Following the right side of the (a) energetic pathway, the hydrogen transfer from a methyl group bonded to the γ carbon cleaves γ and β C−C bond and forms acetaldehyde and prop-1-en-2-ol, with a calculated enthalpy change of 18 kJ/mol (E1*). The barrier of this hydrogen transfer is of 289 kJ/mol (TS1*). The formation of propyne has a calculated transition state barrier of 331 kJ/mol (TS2*). The potential energy surface diagram pathway to the left forms two products identified at signal m/z 56. With a calculated barrier of 268 kJ/mol (TS1) and an enthalpy change of 50 kJ/mol (E1), the epoxide (E) rearranges through a hydrogen transfer to the alcohol group yielding an epoxide + H2O. The epoxide breaks with a barrier of 326 kJ/mol (TS2). A hydrogen transfer to the methylene group initiates the breaking of the epoxide group forming 2-ethacrolein, which is not observed due to poor Franck−Condon factors. E2 converts into E3 with a barrier of 279 kJ/mol (TS3). This species has a calculated adiabatic ionization energy of 8.32 eV. The optimized cation has a slightly different structure than the neutral species, further indicating that the species is not observed due to poor FC factors. From this point, carbon monoxide cleaves off creating a double radical on the β carbon with a calculated heat of reaction of 278 kJ/mol (E4) and no K


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Figure 16. (a) Potential energy surface diagram of the proposed mechanisms of the oxidation of MBO + O(3P). Each energy level throughout this diagram was calculated using the CBS-QB3 method and are all relative to the epoxide (E) at-370 kJ/mol. (b) Potential energy surface diagram continued of the proposed mechanisms of the oxidation of MBO + O(3P) with the epoxide (F) reference point at −370 kJ/mol forming the rest of the products seen in the reaction.

reference level. The intermediate D2 and D4 species in the pathway for propene formation are not observed because D2 dissociatively ionizes and D4 has poor FC factors. 2-Butenal, which is observed experimentally, cannot be yielded via the presented computed potential energy surface because it needs

energy reference level. Cyclobutene is not observed at room temperature but it is formed at 550 and 650 K. The intermediate cyclobutanecarboaldehyde (D3*) is also observed at the higher temperatures. The formation of propene continues from species D1 through the highest TS3 barrier, which is below the energy L


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Figure 17. Potential energy surface diagram of the hydrogen abstraction radical reacting with O2 addition onto radical C for the oxidation of MBO + O(3P) for the formation of propene, cyclobutene, and 2-butenal. The energies throughout these mechanisms were calculated using the CBS-QB3 method and are expressed through radical D.

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to overcome two very high barrier 217 (TS4) and 163 (TS5) kJ/mol higher than the energy reference level.

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Corresponding Author

*(G.M.) E-mail: [email protected].

CONCLUSIONS The biofuel additive, MBO, is oxidized using O(3P) atoms at 298, 550, and 650 K. This study presents the thorough investigation of the low-pressure elementary reactions of this oxidation at different temperatures. The primary products in this study are identified and presented. The experiments are carried out using the synchrotron radiation of the Advanced Light Source (ALS) of the Lawrence Berkeley National Laboratory as the ionization source. At room temperature only three species are identified, ethenol, acetaldehyde, and acetone with a total branching fraction of 84.2 ± 34.8%. At 550 and 650 K more products are observed and the overall branching fractions are 91.6 ± 33.9% and 98.7 ± 17.2%, respectively. Acetone with a branching fraction of 50.4 ± 31.8% is the major product at 550 K, whereas at 650 K trans-2-butene becomes the most abundant product with a branching fraction of 23.1 ± 10.5%. The relative amount of ethenol and acetone diminishes as the temperature is increased. The potential energy surface has been computed using the CBS-QB3 composite model to validate the formation of the observed species.

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AUTHOR INFORMATION

ORCID

Giovanni Meloni: 0000-0003-1697-5104 Notes

The authors declare no competing financial interest.

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ACKNOWLEDGMENTS This work is supported by the Donors of the American Chemical Society Petroleum Research Fund, Grant No. 56067UR6, and the University of San Francisco via the Faculty Development Fund. The authors thank Professors Castro and Karney for their support and use of the USF chemistry computer cluster. The authors would also like to acknowledge Drs. Taatjes and Osborn from Sandia National Laboratories for the use of the experimental apparatus. The Advanced Light Source is supported by the Director, Office of Science, Office of Basic Energy Sciences, of the U.S. Department of Energy under Contract No. DE-AC02-05CH11231.

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(1) Criteria Air Pollutants; United States Envrionmental Protection Agency: Research Triangle Park, NC, 2016. (2) Climate Change: Basic Information; United States Environmental Protection Agency: Washington, DC, 2016. (3) The High Cost of Fossil Fuels; Environment America: Boston, MA, 2016. (4) Huber, G. W.; Iborra, S.; Corma, A. Synthesis of Transportation Fuels from Biomass: Chemistry, Catalysts, and Engineering. Chem. Rev. 2006, 106, 4044. (5) Wyman, C. E. Appl. Biochem. Biotechnol. 1994, 45-46, 897.

ASSOCIATED CONTENT

S Supporting Information *

The Supporting Information is available free of charge on the ACS Publications website at DOI: 10.1021/acs.jpca.6b12421. Optimized molecular structures of species in Figure 16a, 16b, and 17; Cartesian coordinates of optimized molecular structures of species in Figure 16a, 16b, and 17 (PDF) M


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